Ap Chem. Ch. 13 Flashcards
As a solution forms, the solvent pulls solute particles apart and surrounds them.( if its in water, what is this process called?)
Solvation
Homogeneous mixtures( solutions) are formed when 1 _______ disperses uniformly throughout another ______.
Solute
Slovent
In the absense of a strong solvent-solute attraction, the particles randomly spread out. This is typical for nonpolar solutions.
Dispersion
The ability of substances to form solutions depends on 2 factors.
- Type of intermolecular interactions involved
2. Entropy
Natural tendency of substances to spread into larger volumes when not restrained.
Entropy
There are three forces at work during solvation.
- break solvent-solvent attractio
- break solute-solute attraction
- Make solvent-salute attraction
Intermolecular forces that are the strongest when breaking solvent-solvent attraction.
Hydrogen bonding and dipole-dipole
Intermolecular force is the easiest to break in a solvent-solvent attraction.
London forces
Intermolecular forces that are the strongest when breaking solute-solute attraction.
Ionic, metallic
Intermolecular forces that are not as strong and not as weak to break in a solute-solute attraction.
Hydrogen bonding and dipole-dipole
Intermolecular forces that are easiest to break in a solute-solute attraction.
Lodon forces
Intermolecular force is the hardest to break in a solvent-solute attraction.
Ion – dipole, hydrogen bonding, and dipole – dipole
Intermolecular force is the easiest to break in a solvent-solute attraction.
Ion– Induced dipole, dipole – induced dipole, and London forces
Three processes that affects energetics of solution
- Separation of solute particles
- separation of solvent particles
- New interactions between solute and solvent
Separation of solute particles is a________process
Endothermic
Separation of solvent particles is____________process
Endothermic
Interactions between salute installment are a___________process
Exothermic
Things do not tend to occur spontaneously unless …
The energy of the system is lower (overall exothermic)
What does the order of randomness of the system tend to do to the energy of the system ?
Dissolving is therefore what kind of reaction?
It tends to lower the energy
Disolving is a spontaneous reaction
Even though enthalpy may increase,the overall energy of the system can still decrease in the system becomes more what?
Disordered
Physical change – you can get back the original solute by evaporating the solvent
Dissolution
In this type of solution, the solvent holds as much solute as is possible at that temperature
Saturated
In a saturated solution the dissolved solute is in a dynamic__________
with solid solute particles
Equilibrium
In this type of solution less solute that can be dissolved in the solvent at that temperature is dissolved in the solvent.
Unsaturated
This type of solution the solvent holds more solute that is normally possible at that temperature.The solutions are unstable; Crystillization can usually be stimulated by adding a “seed crystal” or scratching the side of the flask.
Supersaturated solution
Like dissolves like states that polar substances tend to dissolve in_________solvents. Nonpolar substances tend to dissolve in________ solvents.
Polar nonpolar
What is the relationship between intermolecular attractions and solubility in water?
The more similar the intermolecular attractions, the more likely one substance is to be soluble in another
The solubility of a gas in a liquid is_________to its pressure.
Directly proportional
Henry’s law
Equation for Henry’s law
S1/P1=S2/P2
Generally, the solubility of solid solutes in liquid solvents_______with increasing temperature. The opposite is true of gases.
Increases
Increasing temperature of the water decreases the ______of the dissolved gases.
Decreases the solubility
Relatively small concentration
Dilute
Relatively larger concentration
Concentrated
Percent mass is also known as….
Known as “PPH”.(Parts per hundred)
Equation for % mass
% mass =mass of A in solution
—————————- x 100
total mass of solution
Mole fraction equation
X = moles of A
A ————–
Total moles in solution
Equation for molarity
M= mol of solute / L of solution
Equation for molality
m = mol of solute / kg of solvent
Since both moles and mass do not change with temperature, molality is not …….
temperature dependent
We can calculate the molality from the molarity and vice versa if we know this thing, what is it?
Density of the solution
Changes in colligative properties depend on the ________ of solute particles present, not the identity of the solute particles.
Number
Among collegative properties are:
Vapor pressure lowering
boiling point elevation
melting point depression
Osmotic pressure
Because of salute – solvent intermolecular attraction, higher concentrations of nonvolatile make it __________for solvents to scape to the vapor phase.
Make it harder
Vapor pressure of a solution ______is then the pure solvent.
Lower
Raoult’s law equation
P = X P°
A A A
Interactions that cost solutions to have higher boiling points lower freezing points than the pure solvent.
Nonvolatile solution – solvent interactions
Net movement of solvent from the area of higher solvent concentration to an area of lower solvent concentration is work.
Osmosis
Pressure required to stop a smosis, known as osmotic pressure,I~I ,is…
I~I = ( n/ V )RT or = MRT
If the osmotic pressure is the same on both sides of the membrane, the solutions are …
Isotonic
The solute concentration outside the cell is greater than that inside the cell, the solution is….
Hypertonic
If the solution is hypertonic then water will flow out of the cell and what results from this?
Crenation
If the solute concentration outside the cell is less than that inside the cell, the solution is…
Hypotonic
If the solution is hypotonic water will flow into the cell and what results from this?
Hemolysis
Suspensions of particles larger than idividual molecules or ions,but too small to be settled out by gravity are called…
Colloids
Colloidal suspensions can scatter rays of light and this phenomenon is known as…
The Tyndall effect
Water loving
Hydrophilic
Water hating
Hydrophobic
Large molecules with the hydrophilic polar groups on the. surface and the hydrophobic portions folded in
Hydrophilic colloid
Hydrophilic colloids can absorb ions in this causes them to be _________by water
Attracted by water
Molecule with polar and nonpolar portions like soap
Emulsifying agents
